Answer
No.
Work Step by Step
We know that the prediction of the wavelengths in the hydrogen absorption spectrum is given by
$$\lambda_{m\rightarrow n}=\dfrac{\lambda_0}{\dfrac{1}{m^2}-\dfrac{1}{n^2}}$$
where $m=1,2,3,..$, and $n=m+1,m+2,m+3,...$
We know that most of the atoms in a gas are in the ground state which means that the only quantum jumps seen in the absorption spectrum start from this state.
Thus, let's set $m=1$, and hence $n=2,3,4,...$
$$\lambda_{1\rightarrow n}=\dfrac{\lambda_0}{\dfrac{1}{1^2}-\dfrac{1}{n^2}}$$
where $\lambda_0=91.18$ nm
$$\lambda_{1\rightarrow n}=\dfrac{91.18}{1-\dfrac{1}{n^2}}$$
Now let's try to find the absorption spectral line with 656.5 nm.
$$\lambda_{1\rightarrow 2}=\dfrac{91.18}{1-\dfrac{1}{2^2}}=\color{green}{\bf 121.6}\;\rm nm$$
$$\lambda_{1\rightarrow 3}=\dfrac{91.18}{1-\dfrac{1}{3^2}}=\color{green}{\bf 102.5}\;\rm nm$$
$$\lambda_{1\rightarrow 4}=\dfrac{91.18}{1-\dfrac{1}{3^2}}=\color{green}{\bf 97.3}\;\rm nm$$
We can see that the wavelengths decrease by increasing $n$ which means that we do not find any spectral line with $\lambda=656.5$ nm.
Therefore, no spectral line with wavelength 656.5 nm is seen in the absorption spectrum of hydrogen atoms.
